Q.1 0.1 mole of which of the reagents listed below[(1)to(6)]could be added to 1 litre of water to make 0.1M solutions of each of the following ions seprately?
(a)NH4^+ (b)CH3COO^- (c)Cl^-
(1) NH3 (2)NH4Cl (3) CH3COOH
(4)CH3COONa (5)HCl (6)NaCl

Why is it important that the sequence of addition of reagents be followed? What could possibly go wrong when this is not followed? Reagents added: 1st: Fe3+ solution 2nd: 2.00 mL 10% NH2OH-HCl (hydroxylamine hydrochloride) 3rd:

Why is it important that the sequence of addition of reagents be followed? What could possibly go wrong when this is not followed? Reagents added: 1st: Fe3+ solution 2nd: 2.00 mL 10% NH2OH-HCl (hydroxylamine hydrochloride) 3rd:

c. A student put 1.18 mole of substance A and and 2.85 mole of substance B into a 10 litre flask which was then closed. The reaction that took place was: A(g)+ 2B(g) 3C(g) + D(g) On analysis the equilibrium mixture at 25 0 C was

Which reagents reagents to choose? The transformation shown below can be accomplished in TWO reaction steps. From the following list, select the two reagents (or sets of reagents) which would most effectively bring about this

I don't know how to start this problem. Someone can help me please. One dm3 of a solution was prepared containing 0.0040 mole of Pb(NO3)2. The Ksp of PbCI2 for the existing conditions is 2.4 x 10^-4. From the list below, choose

I have a test on monday and I NEED to ace it in order to raise my grade > . < ldsfkjaslkf right now, acids and bases are killing me can somebody help me with these problems? A buffer solution is prepared by mixing the weak base

When 0.5 mole of CO2 and 0.5 mole of H2 were forced into a litre reaction container, and equilibrium was established: CO2(g) + H2(g) H2O (g) + CO (g) Under the conditions of the experiment, K=2.00 a) Find the equilibrium